The rate for the reaction $2 A + B \rightarrow \text{product}$ is $6 \times 10^{-4} \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate constant if the reaction is first order in $A$ and zeroth order in $B$,given $[A] = [B] = 0.3 \ M$.

The following data was obtained for the chemical reaction given below at $975 \ K$: $2 NO_{(g)} + 2 H_{2(g)} \rightarrow N_{2(g)} + 2 H_{2}O_{(g)}$

Experiment	$[NO] \ (mol \ L^{-1})$	$[H_{2}] \ (mol \ L^{-1})$	Rate $(mol \ L^{-1} \ s^{-1})$
$1$	$8 \times 10^{-5}$	$8 \times 10^{-5}$	$7 \times 10^{-9}$
$2$	$24 \times 10^{-5}$	$8 \times 10^{-5}$	$2.1 \times 10^{-8}$
$3$	$24 \times 10^{-5}$	$32 \times 10^{-5}$	$8.4 \times 10^{-8}$

The order of the reaction with respect to $NO$ is ..... .

The rate law for the reaction $A^{+} + B^{+} + C \longrightarrow \text{Product}$ is expressed as $\text{Rate} = k[A]^{2}[B]^{1}[C]^{0}$. What is the overall order of the reaction?

For a reaction $A \rightarrow \text{Product}$,the rate constant is $6.93 \times 10^{-3} \ hour^{-1}$. What is the order of the reaction?

Which one of the following statements regarding the order of a reaction is not correct?

Consider the following reactions:
$A$ $\rightarrow P_1; B$ $\rightarrow P_2; C$ $\rightarrow P_3; D$ $\rightarrow P_4$
The orders of the above reactions are $a, b, c,$ and $d,$ respectively. The following graph is obtained when $\log[\text{rate}]$ vs. $\log[\text{conc.}]$ are plotted:
Among the following,the correct sequence for the order of the reactions is: